Question

My question was: A saturated solution of MgF2 at 23 degrees C was prepared by dissolving solid MgF2 in 1 L water. The Ksp of MgF2 is 1.5e-5.
a.)Calculate the mass of MgF2 dissolved.
b.) When .1 mols of solid KF was dissolved in the MgF2 solution, precipitation was observed. Find the mass of the additional precipitate.
I think I get a, I just found the molarity of Mg2+ using the Ksp and then converted to grams; but, I have no idea how to do b. Thanks in advance.

Your answer was: The b part is a common ion problem; i.e., F^- is the ion common to both KF and MgF2.
For part b, Ksp = (Mg^2+)(F^-)^2
The common ion shifts the solubility to the left. MgF2 ==> Mg^2+ + 2F^-
because of Le Chatlier's Principle. The new solubility will = new (Mg^2+) and you can convert that to g MgF2 in the 1L. Subtraction from the initial amount will give you the amount pptd.

New question: I'm sorry but I am still so confused on pretty much everything. How do you calculate the new solubility? And how do you convert that to g MgF2 in 1L? And what is the initial amount that you subtract from?

Answers

You said you understood part a. That's the initial amount of MgF2 dissolved in the 1L of water. You should have done this for part a.
............MgF2 ==> Mg^2+ + 2F^-
I...........solid.....0.......0
C...........solid.....x.......2x
E...........solid.....x.......2x

Ksp = (Mg^2+)(F^-)^2
1.5E-5 = (x)(2x)^2 = 4x^3
x = solubility MgF2 = about 0.016 but you should do it a little more accurately. That works out to approx 0.97grams MgF2/L

For part b you have two things to consider. The F from MgF2 and the F from KF.
(Mg^2+) from MgF2 = x
(F^-) = 0.032 from MgF2 and 0.1 from KF You may want to assume that 0.1 + 0.032 = 0.1 (the easy way but not too accurate) but at least do this first to see what the answer is.
(x)(0.1)^2 = 1.5E-5
x = (Mg^2+) = (MgF2) = about 1.5E-3 M which converts to 0.0934g MgF2. You had about 0.97 dissolved form part a so the difference is what ppts in part b.
I think the assumption is not valid and I believe you should go through the quadratic formula to find (Mg^2+)=(Mg^2+) as above. That quadratic on second thought it isn't a quadratic but a cubic) you get from (Mg^2+)(F^-)^2 = Ksp
1.5E-5 = (x)(2x+0.1)^2
Solve for x, convert to grams/L, subtract from your number from part a and that will be the amount pptd.
Th whole point of these problems is to show you that by adding a common ion you can decrease the solubility of a sparingly soluble salt dramatically.
You can find calculators on the web that will solve a cubic or you can use that assumption (modified of course) so that 0.1 + 0.032 = 0.132 and use that instead of the 0.1 I used above. Hope this helps.

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